Redox and Non-Redox Reactions Redox and Non-Redox Reactions For each of the following reactions, answer: True...
1. Determine if each of the following reactions is a redox reaction, or is not a redox reaction. a. C4H8 (g) + O2 + H20 (g) + CO2 (g) b. HCl (aq) + NaOH (aq) → H20 (1) + NaCl (aq) c. Fe2O3 + H2 → Fe + H2O d. Cu (s) + HNO3 (aq) → Cu(NO3)2 (aq) + NO2 (g) + H20 (1) e. CzHe(g) + 5 O2 (g) → 3 CO2 (g) + 4 H20 (g)
Redox Equations Which of the following reactions are redox reactions? Identify the substance oxidized, the substance reduced, the oxidizing agent, the reducing agent. 1.2 Mg(s) + O2(g) → 2 MgO (s) 2. H SO. (aq) + Al(OH) (aq) → Al(SO.) (aq) + H,O (1) 3. 2 Na (s) + H2O (1) ► 2 NaOH(aq) + H2(g) 4. Cao (s) + CO2(g) → Caco, (s) 5. AgNO, (aq) + NaCl (aq) ► AgCl(s) + NaNO, (aq) Identify the substance oxidized, the...
Redox reactions can be written as two half-reactions 1. Write half-reactions for the following balanced redox reactions. Identify which of the reactants is the oxidizing agent and which is the reducing agent. a. 2 Cd (s) + O2 (g) → 2Cdo (s) b. Mg (s) + HC,H,O2 (aq) → Mg(C2H2O2)2 (aq) + H2 (9) C. Pb (s) + 2Cl2 (g) → PbCl (s) d. Zn (s) + Pb(NO3)4 (aq) → Zn(NO3)2 (aq) + Pb (s) e. 2 Kl (aq) +...
Identify which of the following reactions are redox reactions. 1st attempt Choose one or more: O NaHCO3(aq) + HI(aq) → Nal(aq) +H20(1) + CO2(8) O 3H2(g) + N2(g) → 2NH3(g) C6H12(s) +902(g) + 6H20(g) +6C02 (8) o NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s)
For each of the following balanced redox reactions, identify which elements get oxidized and reduced. Also, ldentify the oxidant and the reductant. 1) 2Cr20 (aq)+3CH,OH(aq) 16H (aq) 3HCO,H(aq)+4Cr(aq)+ 11H20 (1) 2) 2NO -(aq) + H2S(g) + 2H+(aq) →2NO2(g) + S(g) +2H2O (l)
Part IV: Balancing Redox Reactions in Acidic and Basic Solution General rules for balancing redox reactions in acidic or basic solution: 1. Divide the redox reaction into two half-reactions. One that contains the element that gets Oxidized and one that contains the element that gets reduced. 2. Focusing on one half-reaction at a time, balance all non-H and non-0 atoms. 3. Balance the O atoms by adding water molecules to the side with too few oxygens 4. Balance the H...
Use line notation to represent the electrochemical cells for each of the following overall redox reactions. 2Ag+(aq)+Pb(s)→2Ag(s)+Pb2+(aq) 2ClO2(g)+2I−(aq)→2ClO−2(aq)+I2(s) O2(g)+4H+(aq)+2Zn(s)→2H2O(l)+2Zn2+(aq) please help! thank you!!
4. Which of the following reactions involves neither oxidation nor reduction? a. N2(g) + 3H2(g) - 2NH3(8) b. NH.NO(s) - N2(g) + 2H2O(1) c. Cu(s) + 2Ag (aq) → Cu²+(aq) + 2Ag(s) d. 2 Cro. (aq) + 2H*(ag) - Cr2O72- (aq) + H:0() e. CH:(8) + H2(g) - CH (8) 5. The oxidation number of nitrogen given for all the following species is correct except a. NH4 (-2). b. N30 (+1). c. NH2OH (-1). d. HNO, (+3). e. HN; (-1)....
Separate the following redox reactions into half-reactions, and label each half-reaction as oxidation or reduction. Part A Oxidation half-reaction for 2Li(s)+2H+(aq)→2Li+(aq)+H2(g). Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Oxidation half-reaction for 2Ag+(aq)+Be(s)→Be2+(aq)+2Ag(s). Express your answer as a chemical equation. Identify all of the phases in your answer.
Balance each of the following RedOx reactions occurring in basic conditions: Mn2+(aq) + MnO41-(aq) → MnO2(s) Cl2(g) → ClO31-(aq) + Cl1-(aq)